NH4HCO3 + 2H2O 💧⚡→ HNO3 + CO2↑ + 4H2↑
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- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
Electrolysis of aqueous ammonium hydrogencarbonate yields nitric acid, carbon dioxide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
General equation
- Electrolysis of aqueous solution with water as oxidizing agent
- Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4HCO3 | Ammonium hydrogencarbonate | 1 | Reducing | Soluble in water |
| H2O | Water | 2 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HNO3 | Nitric acid | 1 | Oxidized | – |
| CO2 | Carbon dioxide | 1 | – | – |
| 4 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent◆
ΔrG 665.1 kJ/mol K 0.30 × 10−116 pK 116.52
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 853.5 | 665.1 | 631.4 | – |
per 1 mol of | 853.5 | 665.1 | 631.4 | – |
per 1 mol of | 426.8 | 332.6 | 315.7 | – |
per 1 mol of | 853.5 | 665.1 | 631.4 | – |
per 1 mol of | 853.5 | 665.1 | 631.4 | – |
| 213.4 | 166.3 | 157.8 | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent◆
ΔrG 634.72 kJ/mol K 0.63 × 10−111 pK 111.20
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 795.29 | 634.72 | 538.5 | – |
per 1 mol of | 795.29 | 634.72 | 538.5 | – |
per 1 mol of | 397.64 | 317.36 | 269.3 | – |
per 1 mol of | 795.29 | 634.72 | 538.5 | – |
per 1 mol of | 795.29 | 634.72 | 538.5 | – |
| 198.82 | 158.68 | 134.6 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent◆
ΔrG 705.1 kJ/mol K 0.30 × 10−123 pK 123.53
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 778.5 | 705.1 | 2324 | – |
per 1 mol of | 778.5 | 705.1 | 2324 | – |
per 1 mol of | 389.3 | 352.6 | 1162 | – |
per 1 mol of | 778.5 | 705.1 | 2324 | – |
per 1 mol of | 778.5 | 705.1 | 2324 | – |
| 194.6 | 176.3 | 581.0 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent◆
ΔrG 643.10 kJ/mol K 0.22 × 10−112 pK 112.67
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 775.00 | 643.10 | 442.3 | – |
per 1 mol of | 775.00 | 643.10 | 442.3 | – |
per 1 mol of | 387.50 | 321.55 | 221.2 | – |
per 1 mol of | 775.00 | 643.10 | 442.3 | – |
per 1 mol of | 775.00 | 643.10 | 442.3 | – |
| 193.75 | 160.78 | 110.6 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent◆
ΔrG 713.5 kJ/mol K 0.10 × 10−124 pK 125.00
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 758.2 | 713.5 | 2228 | – |
per 1 mol of | 758.2 | 713.5 | 2228 | – |
per 1 mol of | 379.1 | 356.8 | 1114 | – |
per 1 mol of | 758.2 | 713.5 | 2228 | – |
per 1 mol of | 758.2 | 713.5 | 2228 | – |
| 189.6 | 178.4 | 557.0 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 792.5 | – | – | – |
per 1 mol of | 792.5 | – | – | – |
per 1 mol of | 396.3 | – | – | – |
per 1 mol of | 792.5 | – | – | – |
per 1 mol of | 792.5 | – | – | – |
| 198.1 | – | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 775.7 | – | – | – |
per 1 mol of | 775.7 | – | – | – |
per 1 mol of | 387.9 | – | – | – |
per 1 mol of | 775.7 | – | – | – |
per 1 mol of | 775.7 | – | – | – |
| 193.9 | – | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 772.2 | – | – | – |
per 1 mol of | 772.2 | – | – | – |
per 1 mol of | 386.1 | – | – | – |
per 1 mol of | 772.2 | – | – | – |
per 1 mol of | 772.2 | – | – | – |
| 193.1 | – | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous ammonium hydrogencarbonate with water as oxidizing agent
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 755.4 | – | – | – |
per 1 mol of | 755.4 | – | – | – |
per 1 mol of | 377.7 | – | – | – |
per 1 mol of | 755.4 | – | – | – |
per 1 mol of | 755.4 | – | – | – |
| 188.8 | – | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| NH4HCO3 (cr) | -849.4[1] | -665.9[1] | 120.9[1] | – |
| NH4HCO3 (ai) | -824.50[1] | -666.07[1] | 204.6[1] | – |
| NH4HCO3 (aq) | -821.7[1] | – | – | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -849.4 kJ · mol−1
- ^ ΔfG°, -665.9 kJ · mol−1
- ^ S°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -824.50 kJ · mol−1
- ^ ΔfG°, -666.07 kJ · mol−1
- ^ S°, 204.6 J · K−1 · mol−1
- ^ ΔfH°, -821.7 kJ · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1